Textbook-Integrated Guide to Educational Resources

TIGER

A New "Bottom-Up" Framework for Teaching Chemical BondingTami Levy Nahum, Rachel Mamlok-Naaman, Avi Hofstein, and Leeor KronikThis article presents a general framework for bonding that can be presented at different levels of sophistication depending on the student's level and needs. The pedagogical strategy for teaching this model is a "bottom-up" one, starting with basic principles and ending with specific properties.Levy Nahum, Tami; Mamlok-Naaman, Rachel; Hofstein, Avi; Kronik, Leeor. J. Chem. Educ.2008, 85, 1680.

The Correlation of Binary Acid Strengths with Molecular Properties in First-Year ChemistryTravis D. FridgenThis article replaces contradictory explanations for the strengths of different binary acids in first-year chemistry textbooks with a single explanation that uses a BornHaber cycle involving homolyic bond dissociation energies, electron affinities, and ion solvation enthalpies to rationalize trends in the strengths of all binary acids.Fridgen, Travis D. J. Chem. Educ.2008, 85, 1220.

Acids / Bases |

Atomic Properties / Structure |

Aqueous Solution Chemistry |

Physical Properties |

Thermodynamics

Forecasting Periodic Trends: A Semester-Long Team Exercise for Nonscience MajorsJohn TierneyTeams of students in a course for nonscience majors identify trends among the properties of elements in the periodic table, use Excel to plot and produce best-fit equations to describe relationships among those properties, and apply the resulting formulas to predict and justify the properties of missing elements.Tierney, John. J. Chem. Educ.2008, 85, 1215.

More on ClO and Related RadicalsWilliam B. JensenThe novel Lewis structure for the ClO radical and other related 13e isoelectronic species presented by Hirsch and Kobrak is identical to that proposed by Linnett over 40 years ago for the same species on the basis of his well-known double-quartet approach to Lewis structures.Jensen, William B. J. Chem. Educ.2008, 85, 783.

Concept Maps for General Chemistry Boyd L. EarlTwo concept maps have been developed to represent the organization of the material in a first-semester general chemistry course. By providing these maps to students and referring to them in class, it is hoped that the instructor can assist students in maintaining a grasp of the "big picture" during the progress of the course.Earl, Boyd L. J. Chem. Educ.2007, 84, 1788.

Atomic Properties / Structure |

Gases |

Molecular Properties / Structure |

Stoichiometry |

Periodicity / Periodic Table

E = mc2: An Intuitive DerivationJames J. Leary and William H. InghamEinstein's famous equation E = mc2 is derived using a thought experiment that can easily be understood by any serious student of chemistry.Leary, James J.; Ingham, William H. J. Chem. Educ.2007, 84, 1651.

Atomic Properties / Structure |

Instrumental Methods

Lewis Structure Representation of Free Radicals Similar to ClOWarren Hirsch and Mark KobrakAn unconventional Lewis structure is proposed to explain the properties of the free radical ClO and a series of its isoelectronic analogues, particularly trends in the spin density of these species. Hirsch, Warren; Kobrak, Mark. J. Chem. Educ.2007, 84, 1360.

Atmospheric Chemistry |

Computational Chemistry |

Covalent Bonding |

Free Radicals |

Lewis Structures |

Molecular Modeling |

MO Theory |

Valence Bond Theory

Guitar Strings as Standing Waves: A DemonstrationMichael DavisThis demonstration uses an acoustic guitar to produce three unique harmonic vibrations, each of which is representative of a standing wave and illustrates the concept of quantization.Davis, Michael. J. Chem. Educ.2007, 84, 1287.

Mustard Gas: Its Pre-World War I HistoryRonald J. Duchovic and Joel A. VilenskyA review of the history of the synthesis of mustard gas by 19th century European chemists highlights the increasing sophistication of the chemical sciences during this time.Duchovic, Ronald J.; Vilensky, Joel A. J. Chem. Educ.2007, 84, 944.

Applications of Chemistry |

Atomic Properties / Structure |

Toxicology

Aromatic Bagels: An Edible Resonance AnalogyShirley LinDescribes a classroom demonstration involving the use of a bagel and cream cheese as an analogy for benzene that emphasizes the deficiencies of using a single Lewis structure to describe this structure.Lin, Shirley. J. Chem. Educ.2007, 84, 779.

Let Us Give Lewis Acid–Base Theory the Priority It DeservesAlan A. ShafferThe Lewis concept is simple yet powerful in its scope, and can be used to help beginning students understand reaction mechanisms more fully. However, traditional approaches to acid-base reactions at the introductory level ignores Lewis acid-base theory completely, focusing instead on proton transfer described by the Br?nsted-Lowry concept.Shaffer, Alan A. J. Chem. Educ.2006, 83, 1746.

Acids / Bases |

Lewis Acids / Bases |

Lewis Structures |

Mechanisms of Reactions |

Molecular Properties / Structure |

VSEPR Theory |

Covalent Bonding |

Brønsted-Lowry Acids / Bases

Magnet and BB Analogy for Millikan's Oil-Drop ExperimentEarl F. PearsonDescribes the use of refrigerator magnets and BB's as an analogy to Millikan's oil-drop experiment. The mass of a single BB is determined without ever measuring the mass of one BB or determining the mass of a known number of BB's.Pearson, Earl F. . J. Chem. Educ.2006, 83, 1313.

Enrichment / Review Materials |

Atomic Properties / Structure |

Descriptive Chemistry |

Student-Centered Learning

Millikan: Good to the Last (Oil) DropEarl F. PearsonIn this analogy, drop-shaped pieces of magnet represent oil drops, steel BBs represent the electrons, and the mass of a BB represents the charge of an electron. The smallest possible difference in mass between any two samples of BBs should be the mass of a single BB.Pearson, Earl F. . J. Chem. Educ.2006, 83, 1312A.

Atomic Properties / Structure

Lecture Templates: Convenient Partial Lecture Delivery SystemElzbieta Cook and Robert L. CookReports on the use of two forms of PowerPoint lecture presentationsa complete version used by the lecturer and a corresponding partial version available in advance to students. Pre-prepared lecture presentations allow for the sharing of lecture materials among teaching faculty and ensure consistency among several lecture sections in team taught courses.Cook, Elzbieta; Cook, Robert L. J. Chem. Educ.2006, 83, 1176.

Factors That Influence Relative Acid Strength in Water: A Simple ModelMichael J. MoranThe pKa's of diverse aqueous acids HA correlate well with the sum of two gas-phase properties: the HA bond-dissociation enthalpy and the electron affinity of the A radical. It is suggested that rather than bond strength alone or bond polarity, the sum of the enthalpies of these two steps is a fairly good indicator of relative acidity.Moran, Michael J. J. Chem. Educ.2006, 83, 800.

Acrostic Puzzles in the ClassroomDorothy SwainAcrostic puzzles are an effective vehicle to expose students to the history and philosophy of science without lecturing.Swain, Dorothy. J. Chem. Educ.2006, 83, 589.

Atomic Properties / Structure |

Enrichment / Review Materials |

Nomenclature / Units / Symbols |

Nonmajor Courses |

Periodicity / Periodic Table

Probing the Orbital Energy of an Electron in an AtomJames L. BillsThis article answers an appeal for simple theoretical interpretations of atomic properties. A theoretical snapshot of an atom, showing the screened nuclear charge and the electron to be ionized at its radius of zero kinetic energy, enables anyone to approximate its ionization energy.Bills, James L. J. Chem. Educ.2006, 83, 473.

Are Some Elements More Equal Than Others?Ronald L. RichPresents a new periodic chart with 18 columns but no interruptions of atomic numbers at Lanthanum or Actinum, and no de-emphasis of elements 57-71 or 89-103 by seeming to make footnotes of them. It shows some elements more than once in order to illuminate multiple relationships in chemical behavior. Rich, Ronald L. J. Chem. Educ.2005, 82, 1761.

Atomic Properties / Structure |

Descriptive Chemistry |

Inner Transition Elements |

Main-Group Elements |

Nomenclature / Units / Symbols |

Oxidation State |

Periodicity / Periodic Table |

Transition Elements

Trends in Ionization Energy of Transition-Metal ElementsPaul S. MatsumotoExamines why, as the number of protons increase along a row in the periodic table, the first ionization energies of the transition-metal elements are relatively steady, but that for the main-group elements increases.Matsumoto, Paul S. J. Chem. Educ.2005, 82, 1660.

E = mc2 for the Chemist: When Is Mass Conserved?Richard S. TreptowEinstein's famous equation is frequently misunderstood in textbooks and popular science literature. Its correct interpretation is that mass and energy are different measures of a single quantity known as massenergy, which is conserved in all processes.Treptow, Richard S. J. Chem. Educ.2005, 82, 1636.

Atomic Properties / Structure |

Nuclear / Radiochemistry |

Theoretical Chemistry |

Thermodynamics

Measurement of the Isotopic Ratio of 10B/11B in NaBH4 by 1H NMRMurray Zanger and Guillermo MoynaA simple and remarkably accurate method for estimating the isotopic ratio between 10B and 11B through the use of 1H nuclear magnetic resonance (NMR) spectroscopy is presented. The experiment relies on the splitting caused by 10B (I = 3) and 11B (I = 3/2) on the 1H signal of a proton directly bound to boron, a phenomenon readily observed on an aqueous sample of NaBH4. In combination with a brief lecture or prelaboratory presentation, this laboratory can serve to introduce students to magnetic properties as well as theoretical and experimental aspects of NMR spectroscopy as early as the freshman-level chemistry. Zanger, Murray; Moyna, Guillermo. J. Chem. Educ.2005, 82, 1390.

Electronegativity and the Bond TriangleTerry L. Meek and Leah D. GarnerThe dependence of bond type on two parameters, electronegativity difference (??) and average electronegativity (?av), is examined. It is demonstrated that ionic character is governed by the partial charges of the bonded atoms, and metallic character by the HOMOLUMO band gap.Meek, Terry L.; Garner, Leah D. J. Chem. Educ.2005, 82, 325.

Atomic Properties / Structure |

Covalent Bonding |

Metallic Bonding |

Ionic Bonding |

Main-Group Elements

The Meaning of d-Orbital LabelsGuy AshkenaziOrbital labels are the angular part of the wave function, expressed in Cartesian coordinates. The mathematical relation between the labels and the shapes of the orbitals is discussed. Ashkenazi, Guy. J. Chem. Educ.2005, 82, 323.

Atomic Properties / Structure |

Transition Elements |

Quantum Chemistry

Turning on the Light: Lessons from LuminescencePatricia B. OHara, Carol Engelson, and Wayne St. PeterThe goal of this article is to provide secondary school science teachers with a background in an array of luminescent phenomena including fluorescence, phosphorescence, and chemiluminescence that will enable them to teach their students fundamental properties of light and matter. Instructions for building and operating a simple spectrofluorometer and five detailed lesson plans are provided in the Supplemental Material for experiments that utilize these processes. O'Hara, Patricia B.; Engelson, Carol; St. Peter, Wayne. J. Chem. Educ.2005, 82, 49.

Fluorescence Spectroscopy |

Forensic Chemistry |

Photochemistry |

Atomic Properties / Structure

Flame Tests: Which Ion Causes the Color?Michael J. SangerStudents determine which of the ions in a series of ten commercially-available ionic compounds are responsible for the observed colors by performing flame test experiments using cotton swabs and a Bunsen burner.Sanger, Michael J. J. Chem. Educ.2004, 81, 1776A.

Boiling Point versus MassMichael LaingI am very pleased that Ronald Rich has written making these comments, because he is pre-eminent in this field, beginning with his early book, Periodic Correlations.Laing, Michael. J. Chem. Educ.2004, 81, 642.

Atomic Properties / Structure |

Molecular Properties / Structure |

Noncovalent Interactions |

Liquids |

Phases / Phase Transitions / Diagrams

Boiling Point versus Mass Ronald L. RichLaing gave a useful examination of the boiling points of small molecules versus molecular mass. However, a molecule escaping from a liquid is not closely analogous to a satellite breaking free from the earths gravitational field with the requirement of a minimum escape velocity, such that the required kinetic energy is proportional to the mass of the satellite at that escape velocity.Rich, Ronald L. J. Chem. Educ.2004, 81, 642.

A Program of Computational Chemistry Exercises for the First-Semester General Chemistry CourseScott E. Feller, Richard F. Dallinger, and Paul Caylor McKinneyA series of 13 molecular modeling exercises designed for the first-semester general chemistry course is described. The modeling exercises, which are used as both prelecture explorations and postlecture problems, increase in difficulty and in student independence.Feller, Scott E.; Dallinger, Richard F.; McKinney, Paul Caylor. J. Chem. Educ.2004, 81, 283.

Photogalvanic Cells for Classroom Investigations: A Contribution for Ongoing Curriculum ModernizationClaudia Bohrmann-Linde and Michael W. TauschLaboratory experiments examining the fundamental processes in the conversion of light into electrical energy using photogalvanic cells have been developed. These simple cells are suitable for classroom investigations examining the operating principles of photogalvanic cells and the influence of different parameters on their efficiency. Bohrmann-Linde, Claudia; Tausch, Michael W. J. Chem. Educ.2003, 80, 1471.

Electrochemistry |

Atomic Properties / Structure |

Photochemistry |

Oxidation / Reduction |

Electrolytic / Galvanic Cells / Potentials

The KLM-Shell LabelsWilliam B. JensenIn response to a reader's inquiry, this column traces the origins of the K, L, M labels for the shells of the Bohr atom.Jensen, William B. J. Chem. Educ.2003, 80, 996.

The Molecular Model GameStephanie A. MyersStudent teams must draw Lewis structures and build models of various molecules and polyatomic ions; different team members have different responsibilities.Myers, Stephanie A. J. Chem. Educ.2003, 80, 423.

How We Teach Molecular Structure to FreshmenMichael O. HurstExamination of how textbooks discuss various aspects of molecular structure; conclusion that much of general chemistry is taught the way it is for historical and not pedagogical reasons.Hurst, Michael O. J. Chem. Educ.2002, 79, 763.

Response to Lowe's Potential-Energy-Only ModelsLowe, John P.Discussion of the suitability of a potential-only model for the successive ionization energies of sulfur for an introductory chemistry course.Lowe, John P. J. Chem. Educ.2002, 79, 430.

The Mendeleev-Seaborg Periodic Table: Through Z = 1138 and BeyondPaul J. KarolExtending the periodic table to very large atomic numbers and its implications for the organization of the periodic table, consideration of relativistic effects, and the relative stability of massive and supermassive atomic nuclei.Karol, Paul J. J. Chem. Educ.2002, 79, 60.

Lewis Structures in General Chemistry: Agreement between Electron Density Calculations and Lewis StructuresGordon H. PurserThe internuclear electron densities of a series of X-O bonds (where X = P, S, or Cl) are calculated using quantum mechanics and compared to Lewis structures for which the formal charges have been minimized; a direct relationship is found between the internuclear electron density and the bond order predicted from Lewis structures in which formal charges are minimized.Purser, Gordon H. J. Chem. Educ.2001, 78, 981.

Ionization Energies, Parallel Spins, and the Stability of Half-Filled ShellsPeter CannThree methods for explaining the decrease in first ionization energies between group V and group VI elements are described and commented upon. The quantum mechanical origin of the unhelpful concept of half-shell stability is explained in terms of exchange energy, for which the alternative term parallel spin avoidance factor is suggested. It is recommended that for pre-university students the simplest explanation, in terms of Coulombic repulsion between two electrons occupying the same orbital, is adopted: it involves fewer difficult concepts than the other explanations and its predictions are no less accurate. Cann, Peter. J. Chem. Educ.2000, 77, 1056.

Atomic Properties / Structure |

Periodicity / Periodic Table |

Quantum Chemistry |

Theoretical Chemistry

A Drop in the OceanDamon DiementeTeachers of high-school chemistry customarily use calculations done as in-class exercises or as demonstrations to impress their students with the enormity of Avogadro's number and the concomitant miniscularity of atoms and molecules. This article presents and works out one such calculation. Diemente, Damon. J. Chem. Educ.2000, 77, 1010.

Determination of the Fundamental Electronic Charge via the Electrolysis of WaterBrittany Hoffman, Elizabeth Mitchell, Petra Roulhac, Marc Thomes, and Vincent M. StumpoIn an illuminating experiment suitable for secondary school students, a Hoffman electrolysis apparatus is employed to determine the fundamental electronic charge. The volume and pressure of hydrogen gas produced via the electrolysis of water during a given time interval are measured. Hoffman, Brittany; Mitchell, Elizabeth; Roulhac, Petra; Thomes, Marc; Stumpo, Vincent M. J. Chem. Educ.2000, 77, 95.

Atomic Properties / Structure |

Electrochemistry |

Gases |

Molecular Properties / Structure

Analysis of Soft Drinks Using Nuclear Magnetic Resonance Spectroscopy: A MentorshipArkim Wilson, Craig Myers, George Crull, Michael Curtis, and Pamela Pasciak PattersonThis mentorship was designed to expose a student to the laboratory routine for a chemist at Bristol Myers Squibb Company (BMS). The student visited BMS, collaborated with BMS scientists, and actually completed a project on site. He was asked to determine the identity of an unknown sample of soft drink retrieved from a fictitious crime scene using NMR spectroscopy.Wilson, Arkim; Myers, Craig; Crull, George; Curtis, Michael; Pasciak, Pamela M. J. Chem. Educ.1999, 76, 1414.

Instrumental Methods |

Atomic Properties / Structure |

NMR Spectroscopy |

Qualitative Analysis |

Separation Science |

Student / Career Counseling

A Framework for Presenting the Modern AtomJames J. Leary and Tadd C. KippenyA flow chart is presented that summarizes major empirical and theoretical accomplishments that contributed to the modern view of the atom. A chronology is included to show the time dependence of the various contributions. Suggestions are made about how this chart can be used in a variety of contexts as a framework for discussing science as a process.Leary, James J.; Kippeny, Tadd C. J. Chem. Educ.1999, 76, 1217.

Atomic Properties / Structure

Lewis Structures Are Models for Predicting Molecular Structure, Not Electronic StructureGordon H. PurserThis article argues against a close relationship between Lewis dot structures and electron structure obtained from quantum mechanical calculations. Lewis structures are a powerful tool for structure prediction, though they are classical models of bonding and do not predict electronic structure. Purser, Gordon H. J. Chem. Educ.1999, 76, 1013.

The Genius of Slater's RulesJames L. ReedWith only a few modifications a procedure has been developed that yields the one-electron energies for atoms and ions with a level of detail very well suited for instruction in the structure and properties of atoms. It provides for the computation of very reasonable values for such properties as ionization energies, electron affinities, promotion energies, electronic transitions, and even XPS and ESCA spectra. Reed, James L. J. Chem. Educ.1999, 76, 802.

Atomic Properties / Structure |

Quantum Chemistry |

Theoretical Chemistry |

Spectroscopy

The Ubiquitous Metaphors of Chemistry TeachingHerbert BeallThe understanding and the confusion resulting from any scientific metaphor thus have to be considered when it is used. For example, a common chemical metaphor for the electron distribution about an atom is a cloud. Some of the entailments of this metaphor are apt, such as the diffuse nature of a cloud. Others, such as the ability of a cloud to evaporate, are not appropriate. Beall, Herbert. J. Chem. Educ.1999, 76, 366.

Atomic Properties / Structure

Chemistry of the Heaviest Elements-One Atom at a TimeDarleane C. Hoffman and Diana M. LeeA 75-year perspective of the chemistry of the heaviest elements, including a 50-year retrospective view of past developments, a summary of current research achievements and applications, and some predictions about exciting, new developments that might be envisioned within the next 25 years.Hoffman, Darleane C.; Lee, Diana M. J. Chem. Educ.1999, 76, 331.

Chromatography |

Instrumental Methods |

Isotopes |

Nuclear / Radiochemistry |

Separation Science |

Descriptive Chemistry |

Enrichment / Review Materials |

Atomic Properties / Structure

The Gravity of the SituationDamon DiementeThis article presents a few calculations demonstrating that gravitational attraction between atoms is many orders of magnitude weaker than the gravitational attraction between Earth and an atom, and that the gravitational attraction between two ions is many orders of magnitude weaker than the electromagnetic attraction between them. Diemente, Damon. J. Chem. Educ.1999, 76, 55.

Atomic Properties / Structure |

Covalent Bonding |

Noncovalent Interactions

Modeling Nuclear Decay: A Point of Integration between Chemistry and MathematicsKent J. Crippen and Robert D. CurtrightA four-part activity utilizing a graphing calculator to investigate nuclear stability is described. Knowledge acquired through the activity provides background for answering the societal question of using nuclear materials for energy production. Crippen, Kent J.; Curtright, Robert D. J. Chem. Educ.1998, 75, 1434.

Nuclear / Radiochemistry |

Atomic Properties / Structure |

Chemometrics

Orbital Models Made of Plastic Soda BottlesVyacheslav V. SamoshinThe models for demonstration of shape and direction of atomic and molecular orbitals, their overlaps, interactions, and hybridizations may be easily constructed from plastic soda bottles. When the bottles are screwed into the lids, the models of sp3, sp2, or sp hybridized atoms are obtained. Samoshin, Vyacheslav V. J. Chem. Educ.1998, 75, 985.

Molecular Mechanics / Dynamics |

Molecular Modeling |

Atomic Properties / Structure

Percent Composition and Empirical Formula - A New ViewGeorge L. GilbertA new method of obtaining the empirical formula for a compound from its percent composition is proposed. The method involves the determination of a minimum molar mass for the compound based on the percentage of each element, obtaining the lowest common molar mass and using this data to calculate the integer values used in writing the empirical formula. Gilbert, George L. J. Chem. Educ.1998, 75, 851.

Atomic Properties / Structure |

Stoichiometry |

Chemometrics

Demonstrating Electron Transfer and Nanotechnology: A Natural Dye-Sensitized Nanocrystalline Energy ConverterGreg P. Smestad and Michael GratzelA unique solar cell fabrication procedure has been developed using natural anthocyanin dyes extracted from berries. It can be reproduced with a minimum amount of resources in order to provide an interdisciplinary approach for lower-division undergraduate students learning the basic principles of biological extraction, physical chemistry, and spectroscopy as well as environmental science and electron transfer.Smestad, Greg P.; Grtzel, Michael. J. Chem. Educ.1998, 75, 752.

Photochemistry |

Plant Chemistry |

Electrochemistry |

Atomic Properties / Structure |

Dyes / Pigments |

Nanotechnology |

Separation Science |

Spectroscopy

Using Balls of Different Sports To Model the Variation of Atomic SizesGabriel PintoIn this article, an analogy is described about the order of magnitude of the variation of atomic sizes that can be used for discussion in introductory chemistry classes. The order of magnitude of this variation, involving microscopic magnitudes, is difficult for students to imagine.Pinto, Gabriel. J. Chem. Educ.1998, 75, 725.

Atomic Properties / Structure

Experimental 4s and 3d Energies in Atomic Ground StatesJames L. BillsA new definition is given for the effective charge Zf. HF orbital energies e4s and e3d are used in concert with I4s and I3d to answer four questions: Why does the 4s sublevel fill before 3d? Why is ionization easier for 4s than 3d? When 4s23dn has e3d < e4s, why doesn't 4s23dn -> 4s13dn+1? Why are Cr and Cu each 4s13dn+1 instead of 4s23dn? Bills, James L. J. Chem. Educ.1998, 75, 589.

Atomic Properties / Structure

Deducing the Shell Model from Ionization Energies and the Use of Models in Introductory ChemistryRonald J. Gillespie, Richard S. Moog, and James N. SpencerA major objection of Rioux and DeKock is the statement in the authors' earlier paper that electron repulsion is responsible for the relative ionization energies of H and He. The commentators work clearly shows that a quantum mechanical treatment of this problem reveals that kinetic energy considerations play a crucial role in these values. However, although their criticism is appropriate in the context of this more sophisticated QM treatment, it does not in any way invalidate the authors original paper, the goal of which was to provide a model, namely the shell model, for the electronic structure of atoms that is consistent with experimental ionization energies.Gillespie, Ronald J.; Moog, Richard S.; Spencer, James N. J. Chem. Educ.1998, 75, 539.

Atomic Properties / Structure |

Quantum Chemistry |

Theoretical Chemistry

The Crucial Role of Kinetic Energy in Interpreting Ionization EnergiesFrank Rioux and Roger L. DeKockThe experimental ratio of the ionization energies of H and He is 1.81. The authors show that it is not correct to interpret this ratio using a classical Coulombic potential energy model. Rather a quantum mechanical model is required in which both kinetic and potential energy play a role. Rioux, Frank; DeKock, Roger L. J. Chem. Educ.1998, 75, 537.

An Improved Method for Students' Flame Tests in Qualitative AnalysisWilliam D. Bare, Tom Bradley, and Elizabeth PulliamA new method for flame tests to be performed by students is presented. The method involves the use of a hot wire to vaporize the sample,which is subsequently drawn into the flame via the burner air vent. William D. Bare, Tom Bradley, and Elizabeth Pulliam. J. Chem. Educ.1998, 75, 459.

Atomic Properties / Structure |

Atomic Spectroscopy

Simplified Lewis Structure Drawing for Nonscience MajorsBarnabe B. MiburoLewis structures are drawn using a simplified novel method with the following features: 1) the atoms used are brought in carrying all their valence electrons; 2) bonds are created by pairing up valence electrons between the central atoms and peripheric atoms; 3) anions are formed by addition of electrons to single electrons on appropriate atoms, while cations are formed by removal of single electrons.Miburo, Barnabe B. J. Chem. Educ.1998, 75, 317.

Learning Theories |

Lewis Structures |

Nonmajor Courses |

Molecular Properties / Structure

Demonstrations on Paramagnetism with an Electronic BalanceAdolf CortelThe demonstration shows the paramagnetism of common inorganic compounds by measuring the force with which they are attracted by a magnet over the plate of an electronic balance. Cortel, Adolf. J. Chem. Educ.1998, 75, 61.

The Disappearing LiquidH. D. Gesser and Ian WardMixing ethanol and water in a volumetric flask results in a noticeable reduction in the volume of the mixture.Gesser, H. D.; Ward, Ian. J. Chem. Educ.1997, 74, 1357.

Liquids |

Solutions / Solvents |

Atomic Properties / Structure

Getting Close with the Instructional Scanning Tunneling MicroscopeCarl Steven RappThis state-of-the-art instrumentation is making it possible for students to actually view atoms in their own classroom. What is truly amazing, however, is that the ISTM can be set up and atomic resolution images obtained in about an hour.Rapp, Carl Steven. J. Chem. Educ.1997, 74, 1087.

Teaching Chemistry with Electron Density ModelsGwendolyn P. Shusterman and Alan J. ShustermanThis article describes a powerful new method for teaching students about electronic structure and its relevance to chemical phenomena. This method, developed and used for several years in general chemistry and organic chemistry courses, relies on computer-generated three-dimensional models of electron density distributions.Shusterman, Gwendolyn P.; Shusterman, Alan J. J. Chem. Educ.1997, 74, 771.

The Traveling ElectronRichard PendarvisAn analogy is drawn between the location of students on vacation and the probability of finding an electron at some point in space. Students participate in developing the analogy by indicating how far from campus they were during a given vacation period. Pendarvis, Richard. J. Chem. Educ.1997, 74, 396.

Atomic Properties / Structure

Electron Affinities of the Alkaline Earth Metals and the Sign Convention for Electron AffinityJohn C. WheelerIt has been known since 1987, both theoretically and experimentally, that the ion Ca- is stable. It is now certain that Sr-, Ba-, and Ra- are also stable, and accurate values for the electron affinities of Ca-, Sr-, and Ba- have been determined. Recommended values for these electron affinities, in the units commonly employed in introductory texts and with the sign convention used here, are 2.37, 5.03, and 13.95 kJ/mol for Ca, Sr, and Ba, respectively. Wheeler, John C. J. Chem. Educ.1997, 74, 123.

Electronic Configuration Pattern Found in Pascal's TriangleRobert L. DuncanA simple method for revealing the electronic configuration pattern within Pascal's Triangle is discussed. The origin of this unique pattern may be part of a combinatoric and is suggested a link may be made to quantum mechanics. Based on this triangular array an alternate representation of the Periodic Table is presented.Duncan, Robert L. J. Chem. Educ.1996, 73, 742.

Periodicity / Periodic Table |

Quantum Chemistry |

Atomic Properties / Structure

On the Masses of the Fundamental Particles in the Bound StateR. Subramanium, N. K. Goh, and L. S. ChiaA simple computational approach is presented to show that the masses of the fundamental particles are not only lower in the elements but are also different for the various elements. Only basic concepts relating to an atom such as mass number, atomic number, relative isotopic mass, and Avogadro's Number are required.R. Subramanium, N. K. Goh, and L. S. Chia. J. Chem. Educ.1996, 73, 663.

Atomic Properties / Structure

An Approach to Reaction Thermodynamics through Enthalpies, Entropies, and Free Energies of AtomizationJames N. Spencer, Richard S. Moog, and Ronald J. GillespieAn alternative to the conventional method of calculating enthalpies of reaction is presented, using enthalpies of atomization in place of enthalpies of formation. This allows the student to see directly that the reaction enthalpies are determined by the difference in bond strengths in the reactants and products.James N. Spencer, Richard S. Moog, and Ronald J. Gillespie. J. Chem. Educ.1996, 73, 631.

Bonding and Molecular Geometry without Orbitals- The Electron Domain ModelRonald J. Gillespie, James N. Spencer, and Richard S. MoogAn alternative to the conventional valence bond approach to bonding and geometry-the electron domain model-is presented. This approach avoids some of the problems with the standard approach and presents fewer difficulties for the student, while still providing a physical basis for the VSEPR model and a link to the valence bond model.Ronald J. Gillespie, James N. Spencer, and Richard S. Moog. J. Chem. Educ.1996, 73, 622.

Tape and TetrahedraJohn W. HillI have found a simple solution to the problem of visualizing the tetrahedron. I use masking tape or labeling tape to connect the hydrogen atoms to one another. The tape represents the edges of the tetrahedron; the four hydrogen atoms are the corners.Hill, John W. J. Chem. Educ.1996, 73, 531.

Molecular Modeling |

Atomic Properties / Structure |

Molecular Properties / Structure

Glowing VeggiesPirketta Scharlin, Audrey A. Cleveland, Rubin Battino, Monica E. Thomas, and Arnold GeorgeIn this paper we extend our work to other vegetables and the spectra generated by other elements than the sodium in pickle brines. We also did a study on the effect of concentration and voltage on glow intensity.Scharlin, Pirketta; Cleveland, Audrey A.; Battino, Rubin; Thomas, Monica E. J. Chem. Educ.1996, 73, 457.

Conductivity |

Food Science |

Atomic Properties / Structure

A Millikan Oil Drop AnalogyDoris A. EckeyAs an aid to understanding, an analogy is drawn between the manner in which the charge on a single electron is deduced from the total charge on an oil drop, and a rather peculiar pricing system in a surreal candy store.Eckey, Doris. J. Chem. Educ.1996, 73, 237.

Atomic Properties / Structure

A 3-D Diagram of the Relationships among Atomic OrbitalsDonald M. GrahamA stereo diagram is presented of the relationships among the three quantum numbers required to identify atomic orbitals. This provides students with an immediate visual image of the constraints on the values of the quantum numbers. Graham, Donald M. J. Chem. Educ.1996, 73, 210.

Moseley's Work on X-Rays and Atomic NumberC. W. HaighExplanation of the relationship between Moseley's work in determining atomic numbers, the spectrum of the hydrogen atom, the Bohr theory, and Slater's rules for screening constants.Haigh, C. W. J. Chem. Educ.1995, 72, 1012.

Pictorial analogies VII: Quantum numbers and orbitals Fortman, John J.Quantum number n is related to the size of a house, l is related to the shape of a house, and m is compared to the direction the house is facing. Pictures are included.Fortman, John J. J. Chem. Educ.1993, 70, 649.

Electronegativity and atomic chargeReed, James L.Because electronegativity is such a fundamental concept, it should be continually developed in sophistication throughout the curriculum; considers the energy function, atomic charges, and chemical reactivities.Reed, James L. J. Chem. Educ.1992, 69, 785.

The best Aufbau mnemonic: The periodic tableLudwig, Oliver G.Using the periodic table exclusively to rationalize electron assignments has the advantage of emphasizing the experimental aspect of the science and avoids giving the impression that chemistry is nothing but a set of mysterious rules.Ludwig, Oliver G. J. Chem. Educ.1992, 69, 430.

Atomic spectroscopy with a compact disc Mebane, Robert C.; Rybolt, Thomas R.The compact disc used by the music industry provides a convenient and ubiquitous diffraction grating that can be used with a mercury street lamp to explore the electronic structure of atoms through simple atomic spectroscopy observations.Mebane, Robert C.; Rybolt, Thomas R. J. Chem. Educ.1992, 69, 401.

Analogical demonstrations Fortman, John J.By illustrating an analogy with a visual demonstration, a student is aided in both understanding and remembering a lesson.Fortman, John J. J. Chem. Educ.1992, 69, 323.

Close packing of identical spheres Ostercamp, Daryl L.Ordinary marbles can be placed in a wooden rack on the stage of an overhead projector to illustrate the close-pack coordination of 12, the arrangement with 12 nearest neighbor atoms.Ostercamp, Daryl L. J. Chem. Educ.1992, 69, 162.

Explaining resonance - a colorful approachAbel, Kenton B.; Hemmerlin, William M.An analogy using color to help students understand that a resonance molecule does not shift back and forth between Lewis Structures, but is in fact a hybrid of the two structures.Abel, Kenton B.; Hemmerlin, William M. J. Chem. Educ.1991, 68, 834.

MolVib: Visualizing molecular vibrationsHuber, DanielA software program that features animations that aid in visualizing molecular vibrations. This program can be used appropriately in several levels of chemistry.Huber, Daniel J. Chem. Educ.1991, 68, 39.

Simple Inorganic Substances: A New Approach (Sanderson, R.T.)Kauffman, Goerge B.This book stresses the cause-and-effect relationship between the structures of atoms and the properties of their compounds, with an emphasis on providing a thorough understanding of the most familiar and important inorganic compounds.Kauffman, Goerge B. J. Chem. Educ.1990, 67, A26.

Why the Daniell cell works!Martins, George F.The strength of bonds between atoms in metals, the relative ease of removing electrons from atoms, and the energy lowering of the attraction of water molecules for positive ions in solution all aid beginning student's understanding of why reactions occur.Martins, George F. J. Chem. Educ.1990, 67, 482.

Atomic Properties / Structure |

Metals |

Electrolytic / Galvanic Cells / Potentials

Understanding electron configurations Rieck, David F.The author has successfully employed an analogy for understanding electron configurations recommended for use in secondary schools as well as in nonmajor sections of college general chemistry.Rieck, David F. J. Chem. Educ.1990, 67, 398.

Atomic Properties / Structure |

Nonmajor Courses

Magnetic marbles as teaching aidsHill, John W.Magnetic marbles are valuable teaching aids for teachers who have steel chalkboards in their classroom.Hill, John W. J. Chem. Educ.1990, 67, 320.

Atomic Properties / Structure |

Covalent Bonding |

Ion Exchange

The periodicity of electron affinityMyers, R. ThomasIn general, the values of electron affinity for the elements can be understood in terms of their ground state electron configuration, and the screening (effective nuclear charge) exerted on the added electron by the electrons already present in the neutral atom.Myers, R. Thomas J. Chem. Educ.1990, 67, 307.

A student experiment to demonstrate the energy loss and straggling of electrons in matterde Bruin, M.; Huijgen, F. W. J.The experiment described has been applied routinely for several years in introductory courses in the application of radiation and isotopes. The results obtained give direct insight into the characteristics of the phenomena associated with the absorption of energetic electrons in matter.de Bruin, M.; Huijgen, F. W. J. J. Chem. Educ.1990, 67, 86.

Visualization of electron clouds in atoms and moleculesDouglas, John E.110. Visualization of the electron orbital concept continues to challenge and intrigue chemical educators. [October and November 1989 Computer Series both inadvertently called number 107. Numbering restored by skipping 109 and calling January 1990 number 110.]Douglas, John E. J. Chem. Educ.1990, 67, 42.

Atomic Properties / Structure |

Molecular Properties / Structure

Teaching the shapes of the hydrogenlike and hybrid atomic orbitalsAllendoerfer, Robert D.The purpose of this article to show that, in this age of computer graphics, the "difficult to obtain" argument no longer has merit and to give an example of where the standard treatment gives insufficient attention to detail in describing the nodal surfaces of hybrid orbitals.Allendoerfer, Robert D. J. Chem. Educ.1990, 67, 37.

Multiport student spectrometerBishop, Carl B.A spectrometer that can be used simultaneously by seven students to observe a single spectrum emitted by an element of compound in a single light tube against a calibrated screen.Bishop, Carl B. J. Chem. Educ.1989, 66, 1037.

The electronic periodic chart of the elementsvon Marttens Osorio, Hernan; Goldschmidt, AlfonsoA scheme for the arrangement of the elements that allows students to understand and write down the electronic configuration of any given element.von Marttens Osorio, Hernan; Goldschmidt, Alfonso J. Chem. Educ.1989, 66, 758.

What is an element?Roundy, Willard H., Jr.Problems with using outdated definitions of what constitutes an element.Roundy, Willard H., Jr. J. Chem. Educ.1989, 66, 729.

Isotopes |

Atomic Properties / Structure

The historic atom: From d to qSmith, RichardA Styrofoam model of the atom that has been used to show middle and high school students the historical development of the atomic model.Smith, Richard J. Chem. Educ.1989, 66, 637.

A colorful demonstration to simulate orbital hybridizationEmerson, David W.A simple, colorful demonstration involving nothing more than several beakers of colored water can speed up student comprehension of hybrid orbitals at the introductory level.Emerson, David W. J. Chem. Educ.1988, 65, 454.

Principles of electronegativity Part I. General natureSanderson, R. T.The concept of electronegativity has been modified, expanded, and debated. The concept can be used to help students gain valuable insights and understanding of the cause-and-effect relationship between atomic structure and compound properties. This is the first in a series of articles that explores the important concept of electronegativity.Sanderson, R. T. J. Chem. Educ.1988, 65, 112.

Electrochemistry |

Periodicity / Periodic Table |

Noncovalent Interactions |

Atomic Properties / Structure |

Physical Properties |

Enrichment / Review Materials

Orbital plots of the hydrogen atomLiebl, Michael89. Bits and pieces, 36. The software described in this article enable a 48K Apple II with a single disk drive to plot the orbitals of the hydrogen atom in one, two, or three dimensions. This visualization of orbitals allows students to understand their importance in understanding chemistry.Liebl, Michael J. Chem. Educ.1988, 65, 23.

Atomic Properties / Structure |

Quantum Chemistry

Periodic contractions among the elements: Or, on being the right sizeMason, JoanContraction across the row, irregularities in the build up of the periodic table, the second row anomaly relativistic contraction and expansion among the heavier elements, post-transition anomaly, periodicities of physicochemical properties.Mason, Joan J. Chem. Educ.1988, 65, 17.

An upward view of the periodic table: Getting to the bottom of itGuenther, William B.Develops the 18-group basis of the periodic table; shows that, while the 1-18 designations can give unambiguous information to students, no printed designations are needed for teaching; and shows how to obtain unique, physical group definitions that avoid the problems of conflicting and changeable chemical interpretations.Guenther, William B. J. Chem. Educ.1987, 64, 9.

Aufbau on a chessboardHovland, Allan K.A chess or checkerboard offers a convenient frame of reference for a mnemonic to use in writing the electron configuration of the elements.Hovland, Allan K. J. Chem. Educ.1986, 63, 607.

Is an atom of copper malleable?Ben-Zvi, Ruth; Eylon, Bat-Sheva; Silberstein, JudithIt is important to study the mental pictures of the atomic model formed by students at an early stage of their studies, since misunderstanding this model may prevent meaningful learning at later stages.Ben-Zvi, Ruth; Eylon, Bat-Sheva; Silberstein, Judith J. Chem. Educ.1986, 63, 64.

A LAP on moles: Teaching an important conceptIhde, JohnThe objective of the Learning Activity Packet on moles include understanding the basic concept of the mole as a chemical unit, knowing the relationships between the mole and the atomic weights in the periodic table, and being able to solve basic conversion problems involving grams, moles, atoms, and molecules. [Debut]Ihde, John J. Chem. Educ.1985, 62, 58.

Stoichiometry |

Nomenclature / Units / Symbols |

Chemometrics |

Atomic Properties / Structure |

Molecular Properties / Structure |

Periodicity / Periodic Table

Updating the atomic theory in general chemistryWhitman, MarkPresents a descriptive overview of the recent achievements that have furthered the understanding of atomic structure to provide instructors with the background necessary to enhance their classroom presentations.Whitman, Mark J. Chem. Educ.1984, 61, 952.

The use of an air-natural gas flame in atomic absorptionMelucci, Robert C.The experiment reported in this paper demonstrates that students can get excellent results using air-natural gas flame in atomic absorption, and a tremendous advantage in safety is gained for a small sacrifice in the limit of detectability. Melucci, Robert C. J. Chem. Educ.1983, 60, 238.

Atomic Spectroscopy |

Qualitative Analysis |

Metals |

Descriptive Chemistry |

Atomic Properties / Structure

Why doesn't the electron fall into the nucleus?Mason, Franklin P.; Richardson, Robert W.This paper presents a simple, yet essentially correct model of the atom that can be used to answer the title question for even beginning students of chemistry.Mason, Franklin P.; Richardson, Robert W. J. Chem. Educ.1983, 60, 40.

Presenting the Bohr atomHaendler, Blanca L.A more significant consideration of the role of the Bohr theory in the development of quantum mechanics would have many benefits for introductory and advanced chemistry classes.Haendler, Blanca L. J. Chem. Educ.1982, 59, 372.

"The Dancing Wu Li Masters"Stapleton, George W.After reading "The Dancing Wu Li Masters", this author became convinced that the right person can explain the most difficult ideas in a clear, refreshing, and logical manner.Stapleton, George W. J. Chem. Educ.1981, 58, 574.

Quantum Chemistry |

Atomic Properties / Structure

A moir pattern analogy to electron motionBard, James R.The optical illusion produced by this pattern may help students better understand the motion of electrons in atoms.Bard, James R. J. Chem. Educ.1981, 58, 480.

How does the electron cross the node?Johnsen, Russell H.; Lloyd, Winston D.Confusion arises from the assumption that the electron is a particle, when the model that produces an orbital diagram assumes that the electron behaves as a wave.Johnsen, Russell H.; Lloyd, Winston D. J. Chem. Educ.1980, 57, 651.

Empirical formulasRyan, Dennis P.This question forces one to duplicate the line of reasoning used by Dalton in his initial formulation of atomic weights; it tests for the ability to deduce atomic sizes and to calculate empirical formulas.Ryan, Dennis P. J. Chem. Educ.1979, 56, 528.

Using the Aufbau principle Whitmer, John C.This question is written with the belief that general chemistry students should not only attain an understanding of the Aufbau principle enabling them to write down electron configurations, they ought also recognize the correspondence between the quantum numbers and the structures of the periodic table.Whitmer, John C. J. Chem. Educ.1978, 55, 515.

But if atoms are so tiny...Kolb, DorisReviews the atomic theory, the laws of chemical combination, atomic weight scales, Avogadro's hypothesis, the development of the mass spectrograph, the meaning of atomic weight, and the difference between mass and weight in answering the question "If atoms are so small, how can we know how much they weigh?" [Debut]Kolb, Doris J. Chem. Educ.1977, 54, 543.

Chemical aspects of Bohr's 1913 theoryKragh, HelgeThe chemical content of Bohr's 1913 theory has generally been neglected in the treatises on the history of chemistry; this paper regards Bohr as a theoretical chemist and discusses the chemical aspects of his atomic theory.Kragh, Helge J. Chem. Educ.1977, 54, 208.

What is oxidation?Herron, J. DudleyWhy do most teachers continue to define oxidation and reduction in terms of a gain and loss of electrons rather than in terms of a change in oxidation number? [Debut]Herron, J. Dudley J. Chem. Educ.1975, 52, 51.

Line spectrum demonstration for the large lecture hallDriscoll, Jerry A.The undergraduate's learning experience with quantum mechanics and Bohr's theory can be greatly enhanced by the presentation of a line spectrum demonstration, but these are often hard to see in large lecture halls. The authors present a physical arrangement of an apparatus that can be easily assembled to allow for easier student viewing in a lecture-hall situation.Driscoll, Jerry A. J. Chem. Educ.1974, 51, 97.

The stability of the hydrogen atomRioux, FrankThe Kimball-Neumark-Kleiss model of the atom is conceptually correct, requires only simple mathematics, and clearly explains the stability of the hydrogen atom.Rioux, Frank J. Chem. Educ.1973, 50, 550.

Atomic Properties / Structure

Electron affinity. The zeroth ionization potentialBrooks, David W.; Meyers, Edward A.; Sicilio, Fred; Nearing, James C.It is the purpose of this article to present the merits of adopting the terminology zeroth ionization potential to describe the energy change that occurs when a gaseous anion loses an electron.Brooks, David W.; Meyers, Edward A.; Sicilio, Fred; Nearing, James C. J. Chem. Educ.1973, 50, 487.

Aufbau principle: A simple model for demonstrationSagi, Seetarama RajuThis electrical model of the atom used light bulbs to illustrate how the electron density gradually increases around the nucleus with successive additions of electrons to the various orbitals.Sagi, Seetarama Raju J. Chem. Educ.1970, 47, 648.

Atomic Properties / Structure |

Periodicity / Periodic Table

Forces and quantum field theoryBrescia, FrankThis article seeks to explain the nature of forces between nucleons in terms of the quantum field theory for the general reader using a simple analogy.Brescia, Frank J. Chem. Educ.1970, 47, 642.

Interpretation of oxidation-reductionGoodstein, Madeline P.Presents an interpretation of the oxidation number system based upon the electronegativity principle, thus removing the adjective "arbitrary" frequently found in the descriptions of oxidation number.Goodstein, Madeline P. J. Chem. Educ.1970, 47, 452.

Role of f electrons in chemical bindingJohnson, O.Data presented suggests that f electrons, by their ineffective screening of the nuclear charge, exert an indirect effect on the binding strength of actions.Johnson, O. J. Chem. Educ.1970, 47, 431.

High school coursesBriggs, A. G.The author points out that students may be more accepting of chemistry content (such as the size of the atom) if they are allowed to experiment for themselves.Briggs, A. G. J. Chem. Educ.1969, 46, 700.

The five equivalent d orbitalsPowell, Richard E.Several textbooks assert that there is no way of choosing the five d orbitals so they have the same shape but differ only in their orientation.Powell, Richard E. J. Chem. Educ.1968, 45, 45.

Electronegativities and group IVA chemistryPayne, Dwight A., Jr.; Fink, Frank HallThe teacher of inorganic chemistry should present the representative elements of group IVA and their properties as an intellectual and empirical form of investigation rather than as a mere collection of information.Payne, Dwight A., Jr.; Fink, Frank Hall J. Chem. Educ.1966, 43, 654.

Atomic orbitals: Limitations and variationsCohen, Irwin; Bustard, ThomasThe three most widely used methods of arriving at a set of atomic orbitals afford respective hydrogen-like orbitals, self-consistent field orbitals, and various analytical approximations such as the Slater or Morse orbitals, all of which may differ greatly in shape and size from each other.Cohen, Irwin; Bustard, Thomas J. Chem. Educ.1966, 43, 187.

Atomic Properties / Structure |

Quantum Chemistry

General chemistry exercise using atomic and molecular orbital modelsWalker, Ruth A.Styrofoam balls and pipecleaners are used to construct models designed to convey an understanding of the three-dimensionality of the electron distribution in the ground state atom and the effect of bonding on this distribution.Walker, Ruth A. J. Chem. Educ.1965, 42, 672.

LettersGates, Henry S.Brings the reader's attention to work done by Petit and Dulong in revising a large number of atomic weights in order to bring all of their reported atomic heat capacities into agreement with the hypothesis that atomic heat capacity is the same for all elements.Gates, Henry S. J. Chem. Educ.1964, 41, 575.

Energy level diagrams and extranuclear building of the elementsKeller, R. N.Simplified diagrams showing the approximate order of electronic energy levels in atoms and mnemonic devices to aid in predicting electronic configurations for atoms are often misleading with respect to the actual energy of binding of the electrons in atoms and ions of the transition elements.Keller, R. N. J. Chem. Educ.1962, 39, 289.

Molecular models featuring molecular orbitalsBrumlik, George C.Molecular models have been constructed that attempt to represent atomic and molecular orbitals as accurately as the current theories of valence and pertinent experimental evidence permit.Brumlik, George C. J. Chem. Educ.1961, 38, 502.

Molecular Modeling |

Atomic Properties / Structure |

MO Theory

Paddle-wheel Crookes tubeCampbell, J. A.The effect in the Crookes paddle-wheel tube is the same as in the light radiometer and should be interpreted in the same way.Campbell, J. A. J. Chem. Educ.1961, 38, 480.

There are electrons in atoms!Sementsov, A.The author suggests a demonstration of the Zeeman effect to give students real and convincing proof that atoms contain electrons.Sementsov, A. J. Chem. Educ.1961, 38, 22.

Atomic Properties / Structure

The shape of the 2p and related orbitalsCohen, IrwinSome texts mistake graphs of the angular variation of the 2p and related wave functions for actual geometric descriptions of these orbitals.Cohen, Irwin J. Chem. Educ.1961, 38, 20.

Valence: A laboratory exercise for general chemistrySanderson, R. T.In this exercise, each student carefully examines each of a set of thirteen different atomic models with different valence configurations, writing down certain pertinent observations and independently-reasoned conclusions about them.Sanderson, R. T. J. Chem. Educ.1960, 37, 261.

Models for demonstrating electronegativity and "partial charge"Sanderson, R. T.Describes a three-dimensional set of atomic models arranged periodically to illustrate trend in electronegativity and the use of molecular models to illustrate important concepts in general chemistry. Sanderson, R. T. J. Chem. Educ.1959, 36, 507.

A demonstration model illustrating the aufbau principleEverett, D. H.Describes the construction of a physical device capable of illustrating the relationship between the relative energies of electron orbitals in many-electron atoms, the electronic structure of atoms, and the periodic table.Everett, D. H. J. Chem. Educ.1959, 36, 298.

The principle of minimum bending of orbitalsStewart, George H.; Eyring, HenryThe authors present a theory of valency that accounts for a variety of organic and inorganic structures in a clear and easily understood manner.Stewart, George H.; Eyring, Henry J. Chem. Educ.1958, 35, 550.

Atomic Properties / Structure |

Molecular Properties / Structure |

Elimination Reactions

A schematic representation of valenceSanderson, R. T.This paper describes a new chart representing the valence structure of atoms; by studying this chart, with the help of a few simple rules, students of elementary chemistry can acquire a useful understanding of chemical combination.Sanderson, R. T. J. Chem. Educ.1958, 35, 541.

Atomic Properties / Structure |

Periodicity / Periodic Table |

Enrichment / Review Materials |

Transition Elements |

Metals |

Nonmetals

Teaching electron configurationsEichinger, Jack W., Jr.Time can be saved and confusion avoided by developing a systematic chart of the elements based on the energy levels of atomic orbitals very early in the general college chemistry course.Eichinger, Jack W., Jr. J. Chem. Educ.1957, 34, 504.

A helical periodic tableRice, William E.A three-dimensional representation of the periodic table can provide an additional coordinate to represent the difference between subgroups without disrupting the vertical sequence of elements in a whole group.Rice, William E. J. Chem. Educ.1956, 33, 492.

Periodicity / Periodic Table |

Atomic Properties / Structure

Letters to the editorFoster, Laurence S.Thanks a reader for pointing out a misstatement in an earlier article involving atomic mass units and avograms.Foster, Laurence S. J. Chem. Educ.1956, 33, 477.

A new periodic chart with electronegativitiesSanderson, R. T.This paper describes a new chart that has been designed to portray clearly and vividly patterns in relative atomic radius, electronic configuration, and electronegativity.Sanderson, R. T. J. Chem. Educ.1956, 33, 443.

Periodicity / Periodic Table |

Atomic Properties / Structure

A new periodic table based on the energy sequence of atomic orbitalsWalker, W. R.; Curthoys, G. C.Since the theory of atomic and molecular orbitals has proven to be of such value in interpreting the data of inorganic chemistry, it is hoped that a new periodic table based on the energy sequence of atomic orbitals will be an aid to the further systematizing of chemical knowledge.Walker, W. R.; Curthoys, G. C. J. Chem. Educ.1956, 33, 69.

Atomic-weight variations in natureBoggs, James E.Atoms of the same element may have different masses (due to isotopic differences) depending on their source.Boggs, James E. J. Chem. Educ.1955, 32, 400.

The lecture demonstration of atomic spectraWendlandt, Wesley W.Suggests the use of railway or highway flares of different colors to demonstrate the atomic spectra of strontium, barium, or sodium.Wendlandt, Wesley W. J. Chem. Educ.1955, 32, 9.

A cut-out chart of the periodic systemClauson, Jennie E.Colored discs in a cylinder of transparent plastic represent the arrangement of elements in the periodic table. Also provides a chart that can be cut out and turned into a similar cylinder.Clauson, Jennie E. J. Chem. Educ.1954, 31, 550.

Atomic structure and the photoelectric effectBrockett, Clyde P.The ubiquitous and inexpensive 110-volt, 2-watt neon glow lamp appears to have been overlooked as a device well suited to a brief but telling demonstration of a few key principles of atomic structure that underlie the study of electrovalence and comparative chemistry.Brockett, Clyde P. J. Chem. Educ.1953, 30, 498.

Atomic Properties / Structure

An introduction to the electron theory of metalsLefever, Robert A.This discussion is intended to provide a general background for the understanding of metal physics as well as a basis for more advanced study.Lefever, Robert A. J. Chem. Educ.1953, 30, 486.

Demonstration of the intermediate position of cobalt between iron and nickelGoldstein, Ernst M.The different oxidizability of ferrous, cobaltous, and nickelous hydroxides, together with increasing color deepness of the oxidation products, can be used to demonstrate that cobalt is intermediate in its properties between iron and nickel.Goldstein, Ernst M. J. Chem. Educ.1953, 30, 387.

Periodicity / Periodic Table |

Metals |

Oxidation / Reduction |

Atomic Properties / Structure |

Qualitative Analysis

LettersNair, C. N.A mathematical derivation demonstrating that masses of different elements equal to their atomic weights must contain the same number of atoms.Nair, C. N. J. Chem. Educ.1953, 30, 155.

The long form of the periodic tableGlockler, George; Popov, A. I.The authors comment on the independent publication of a periodic table similar to one they produced earlier.Glockler, George; Popov, A. I. J. Chem. Educ.1952, 29, 358.

The periodic table: The 6d-5f mixed transition groupCoryell, Charles D.With relatively few modifications, the Bohr-type periodic table presented by Glocker and Popov can be made to reflect more instructively the rather complex relationships obtained in the neighborhood of the 4f or gadolinium transition group and, more importantly, in the 6d-5f sequence extending from actinium through the region of uranium and the synthetic earths to element 103.Coryell, Charles D. J. Chem. Educ.1952, 29, 62.

Periodicity / Periodic Table |

Transition Elements |

Atomic Properties / Structure

An atomic structure modelHerron, Fred Y.Presents the design of a physical model intended to illustrate the manner in which the electronic configurations of the various elements may be produced by adding electrons to a hydrogen atom.Herron, Fred Y. J. Chem. Educ.1951, 28, 473.